Calculate pV2+ at each of the points in the titration of 21.17 mL of 0.0364 M EDTA with 0.0182 M VCl2 . The EDTA solution is buffered at a pH of 10.00 . The fraction of free EDTA in the Y4− form ( ?Y4− ) can be found in this table. The formation constant for the V2+−EDTA complex is given by log?f=12.7 .
4.234 mLpV2+=
16.94 mLpV2+=
33.87 mLpV2+=
41.49 mLpV2+=
42.26 mLpV2+=
42.34 mLpV2+=
42.42 mLpV2+=
46.57 mLpV2+=
50.81 mLpV2+=
ANSWER:
Data:
Titration reaction:
For the titration:
Dissociation of VY-2:
The equivalence volume (VV+2) is:
Before equivalence point:
Vol V+2 | [EDTA] | [VY-2] |
4.234 mL | ||
16.94 mL | ||
33.87 mL | ||
41.49 mL | ||
42.26 mL |
then
Vol V+2 | [V+2] | pV+2 |
4.234 mL | ||
16.94 mL | ||
33.87 mL | ||
41.49 mL | ||
42.26 mL |
At equivalence point (42.34 mL):
V+2 | + | EDTA | <--> | VY-2 | |
Initial | 0 | 0 | 1.21x10-3 | ||
Final | X | X | 1.21x10-3 - X |
then
the great value of Kf allows this approximation:
then
After equivalence point:
then
Vol V+2 | [V+2] | pV+2 |
42.42 mL | ||
46.57 mL | ||
50.81 mL | |
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